Video 5 and 6 20. The solubility product constant (Ksp) of nickel (II

Video 5 and 6
20. The solubility product constant (Ksp) of nickel (II) carbonate in water at 25o C is
1.3 x 10-7.
a. Write the balanced chemical equation for this dissolving process.
b. Write the equilibrium expression.
c. Find the maximum molar concentration of all ions in solution and the molar solubility of the
solution.
21. The solubility product constant (Ksp) for calcium hydroxide is 6.5 x 10-6 at 25o C.
a. Write the balanced chemical equation for this dissolving process.
b. Write the equilibrium expression.
c. Find the maximum molar concentration of all ions in solution and the molar solubility of the
solution.
d. Calculate the maximum mass of calcium hydroxide that will dissolve in 100 mL distilled water.
22. At a certain temperature, 9.5 x 10-5 grams of zinc carbonate will dissolve in 150 mL of water.
a. Write the balanced chemical equation for this dissolving process.
b. Calculate the molar solubility of zinc carbonate in water at this temperature.
c. Calculate the value of the solubility product constant, Ksp, for zinc carbonate.
23. After 20.0 g of Na2SO4 has been added to a 0.5 L saturated solution of CaSO4, does the concentration of
Ca2+ increase, decrease, or stay the same? Justify your answer. Assume that the overall volume of the
solution does not change.
24. After 31.0 g of NaCl has been added to a 1.0 L saturated solution of PbCl 2, does the concentration of
Pb2+ increase, decrease, or stay the same? Justify your answer. Assume that the overall volume of the
solution does not change.
25. Is CaSO4 more soluble in 1.0 L of 0.25 M Li2SO4 or 1.0 L of 0.25 M Al2(SO4)3? Explain.
26. The solubility product constant, Ksp, for barium sulfate is 1.1 x 10-10 at 25oC. Will a precipitate of BaSO4
form when 210 mL of 4.75 x 10-2 M Ba(NO3)2 is mixed with 315 mL of 0.450 M Li2SO4?
27. For MgF2, Ksp = 6.4 x 10-9, if you mix 500 ml of 1.0 x 10-4 M Mg( NO3)2 and 500mls of 1.00 x 10-4 M NaF,
what will be observed?
28. For CaCrO4, Ksp= 7.1 x 10-4. How many grams of Na2CrO4 must be added to 200.0 mls of 0.250 M
Ca(NO3)2 to begin to see a precipitate form?
29. The solubility of iron (II) hydroxide, Fe(OH)2 is 1.43 x 10-3 grams per liter at 25 oC.
a. Write the balanced equation for the solubility equilibrium
b. Write the expression for the solubility product constant, Ksp, and calculate its value.
c. Calculate the pH of a saturated solution of Fe(OH)2 at 25 oC.
d. A 50.0 milliliter sample of 3.00 x 10-3 M FeSO4 solution is added to 50.0 milliliters of 4.00 x 10-6
molar NaOH solution. Does a precipitate of Fe(OH)2? Explain and show calculations to support
your answer.
30. A saturated solution of lead iodate in pure water has a lead ion concentration of 4.0 x 10 -5 mole per
liter at 20oC.
a. Calculate the value for the solubility product constant of Pb(IO3)2 at 25oC
b. Calculate the molar solubility of Pb(IO3)2 in a 0.10 molar Pb(NO3)2 solution at 25oC
c. To 333 milliliters of a 0.120-molar Pb(NO3)2 solution, 667 milliliters of 0.435-molar KlO3 is
added. Calculate the concentrations of Pb2+ and IO3- in the solution at equilibrium at 25oC
31. If a 0.50 M solution of KOH is slowly poured into a beaker containing 0.35 M magnesium nitrate and
0.32 M calcium nitrate at 25 oC, what will be the first precipitate that forms? Ksp for calcium hydroxide
is 6.5 x 10-6 and Ksp for magnesium hydroxide is 6.3 x 10-10,

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